Chapter 1 Basic Concept of Periodic Table - Online...1.1 Periodic Table 1.2 Periodicity of Properties As per modern periodic law, physical and chemical properties of the element are

Kaysons Education Basic Concept of Periodic Table

Page 1

Day - 1

Periodic Table 1. Classification of Element and Periodicity in Properties

Periodic table may be defined as the table which classifies the entire known element in accordance

with their properties in such a way that element with similar properties are grouped together in the

same vertical columns and dissimilar element are separated from one another.

1.1 Periodic Table

1.2 Periodicity of Properties

As per modern periodic law, physical and chemical properties of the element are a periodic

function of their atomic number i.e., if the element are arranged in order of their increasing atomic

number the element with similar properties are repeated after certain regular intervals.

1.3 Cause of Periodicity

The main cause of periodicity in property is the repetition of similar outer electronic configuration

after certain regular intervals.

Basic Concept of Periodic

Table

Chapter

1


Page 2

1.4 Electronic Configuration of alkali Metals

SYMBOL ATOMIC

NUMBER

ELECTRONIC CONFIGURATION

Li 3

Na 11

K 19

Rb 37

Cs 55

Fr 87

1.5 Electronic Configuration of Halogens

ELEMENT ATOMIC

NUMBER

ELECTRONIC CONFIGURATION

F 9

Cl 17

Br 35

I 53

At 85

One most important point is that there is a repetition in the electronic configuration of noble gases

i.e., regular intervals being 2,8,8,18,18,32 these number are termed as magic number.

1.6 IUPAC Nomenclature Elements with at Number > 100

Roots for IUPAC nomenclature of elements.

DIGIT ROOT ABBREVIATION

0 nil n

1 un u

2 bi b

3 tri t

4 quad q

5 pent p

6 hex h

7 sept s

8 oct o

9 enn e

Z (At. No.) Recommended Name Symbol 101 Unnilunium ( Un + nil + un + ium ) Unu

102 Unnilbium (Un + nil + bi + um) Unb

103 Unniltrium Unt

104 Unnilquadium Unq

105 Unnilpentium Unp


Page 3

106 Unnilhexium Unh

107 Unnilseptiun Uns

108 Unniloctium Uno

109 Unnilennium Une

110 Ununnilium Uun

111 Unununium Uuu

112 Ununbium Uub

113 Ununtrium Uut

114 Ununquadium Uuq

115 Ununpentium Uup

116 Ununhexium Uuh

117 Ununseptium Uus

118 Ununoctium Uuo

119 Ununenium Uue

120 Unbinilium Ubn


Page 4

Self Efforts

1. The elements of group 1, 2, 13, 14, 15, 16, 17, 18 are collectively called

(A) Noble elements (B) Typical elements

(C) Transition elements (D) Representative elements

2. The 3rd

period of the periodic table contains

(A) 8 elements (B) 32 elements

(C) 3 elements (D) 18 elements.

3. Which of the following element does not belong to the family indicated ?

(A) Coinage metal (B) Alkaline earth

(C) Alkaline earth (D) Noble gases.

4. Pd has exceptional configuration 4d10

5s0. It belongs to

(A) 4th

period (B) 6th

period

(C) 7th

period (D) 5th

period.

5. The tenth element in the periodic table resembles the element with atomic number

(A) 2 as well as 30 (B) 2 as well as 54

(C) 8 as well as 18 (D) 8 only.

6. Which of the following sequence contain atomic number of only representative elements?

(A) 3, 53, 33, 87 (B) 13, 33, 54, 83

(C) 22, 23, 66, 54 (D) 3, 13, 48, 53.

7. Which of the following set of species contains elements which have been named in honour of some

countries?

(A) Ge, Bk, Cf (B) Cf, Am, In

(C) Na, Hg, Cf (D) Ru, Am, Ge.

8. According to IUPAC norms a newly discovered element has been named as Uum. The atomic number of

the element is

(A) 111 (B) 112

(C) 109 (D) 110.

ANSWERS

1. D 2. A 3. C 4. D

5. B 6. A 7. D 8. D


Page 5

Day - 2

1. Main Characteristics of Periodic Table

(I) Periods

7 periods.

⟶ 2 Elements H, He (Noble gas) shortest period

⟶ 8 Elements, Be, C, N, O, F, Ne, (Noble gas)

⟶ 8 Elements, Na, Mg, Al, Si, P, S, Cl, Ar, (Noble gas)

⟶ 18 Elements, (First long period) ( Z = 19 to 36)

⟶ 18 Elements, (Z = 37 – 54) Rb = 37 and Xe = 54 Z = 39 – 48 = Transition

Elements

⟶ 32 Elements, (Z = 55 – 86) (55, 56, and 81 – 86) 8 = Normal/representative

Element

(Z = 57, 72 – 80) 10 = Transition Element

Inner transition/Lanthanides (Z = 58 – 71) 14 = Rare Earth Element (Longest period)

⟶ Expected 32 elements but incomplete. (Z = 86 – 62), elements after Ac, i.e.,

from Thorium (90) ⟶ Lawrencium (103) = actinides/rare Earth Elements.

Rare Earth Elements ⟶ are also termed as f – block elements.

Elements beyond Uranium which have been prepared artificially by nuclear reaction called

Transuranic Elements.

(II) Groups

18 Groups,

1.1 Division of Elements into s, p, d, and f block elements

(i) s – block elements

Element in which last electrons enter into s – orbital are termed as s-block elements.

1.2 General Properties

Soft metal with low m. p., low ionization enthalpies, highly electropositive, so reactive

K Kr

Kaysonseducation Metallurgy

Page 24

Day - 1

1. Ores and minerals

Elements are basic units of all types of matter in this universe. Elements are found to occur in

nature either in the free state (native state) or in combined state (ores & minerals).

Important:- All ores are minerals but all minerals are not ores.

Metallurgy

Chapter

2


Page 25

Percentage distribution (by weight) of the most elements in the earth’s crust.

1.1 Principal Minerals/Ores of some important metals

S.

No.

Metal Minerals Chemical formula

1. Aluminium Bauxite

Kaolinite (a form of clay)

(sometimes)

or

2. Iron Haemetite

Magnetite

Siderite

Irom pyrite

3. Copper Copper pyrites

Malachite

Cuprite

Copper glance / Chalcocite

4. Zinc Zinc blend or Sphalerite

Calamine

Zincite

5. Lead Galena

Cerrusite

Anglessite

6. Tin Tinstone or Cassiterite

7. Silver Argentite (Silver glance)

Horn Silver

Pyrargyrite (Ruby Silver)

8. Magnesium Carnalite

Epsomite

Small amount in sea water

Magnesite

Ollvine

Asbestos

Serpentine

In minerals springs

(in sea water)

1.2 Extractive Metallurgy

The process of extracting metals from their ores is called Metallurgy. The metallurgy involves

following processes

1. Crushing & grinding of ore Just to broken the lumps of ores.

2. Concentration or benefaction of ore The removal of unwanted earthy and siliceous impurities

(gangue / matrix) from the ore is ore-dressing or concentration of ore. The process used to

concentrate the ore benefaction process.

3. Extraction of crude metal from concentrated ore.

4. Refining of ore.


Page 26

1.3 Concentration of ore

1. Hydraulic washing / Levigation / Gravity Saperation

Method is used when the ore particles are heavier than the earthy or racky particle. The

process is carried out in specially designed tables called Wilgley tables.

Ex:- Oxide ore of Iron (haemelite), tin nature ore of Ag, Au etc.

2. Electromagnetic Saperation

Method is employed when either ore or impurities associated with it are magnetic in

nature.

Chromite , Magnetite and pyrolusite

= ore of Mn] being separated from non-magnetic silicious gangue.

Tinestone / cassiterite an ore of tin being non-magnetic separated from

magnetic impurities like tungstates of iron and Mn.

3. Froth Floatation Method

Used for sulphide ores

Principle

Surface of sulphide ores is preferentially wetted by oil while that of gangue is

preferentially wetted by water.

Working

The crushed ore mixed with water (in form of suspension) in a tank added collectors (pire

oil, xanthats and fatty acids) which enhance the non-wettability of the ore particles and

froth-stabilizers (Ex. Cresol & aniline) which stabilize the froth. The suspension is

violently agitated by the rotating paddle which draws in air causing frothing. During this

process, the ore particle becomes lighter and thus rise to the surface along with froth

while gangue particles becomes heavier (wetted by water) & thus settle down at the

bottom of tank. The froth is skimmed off, allowed to collapse and finally dried to the

concentrated ore.

If the minerals to be concentrated consists of sulphides of two metals, then by adjusting

the proportion of oil: water, it is often possible to separate ore sulphide from the other.

Depressants are used to prevent one type of sulphide ore particle from forming froth

air bubble.

On surface of ZnS Depressant


Page 27

On surface of ZnS prevent the ZnS for the froth floatation. Only PbS form froth.

4. Leaching/Hydrometallurgy

Treating the powdered ore with a suitable reagent (eg. Acids bases or other chemicals)

which selectivety dissolve ore form soluble complexes but not impurity.

For:- Ag

or

For:- Gold

Sod. Dicyanoargentate (I)

Pot. Dicyanoargentate (I)


Page 28

Self Efforts

1. In the floatation process for the purification of minerals the particles float because

(A) they are light

(B) they are insoluble

(C) their surface is preferentially wetted by oil

(D) they bear an electrostatic charge.

2. Froth floatation process for the concentration of ores is an illustration of the practical application of

(A) Adsorption (B) Absorption

(C) Coagulation (D) Sedimentation.

3. Which method is used for the purification of Bauxite ore ?

(A) Levigation (B) Leaching

(C) Electrolysis (D) Magnetic separation.

4. The process by which lighter earthly particles are freed from the heavier particles by washing with water

is called

(A) Benefication (B) Levigation

(C) Leaching (D) None of these.

5. The most abundant element on earth crust is

(A) H2 (B) O2

(C) Si (D) C.

6. Which of the following is not an ore of magnesium ?

(A) Carnalite (B) Dolomite

(C) Gypsum (D) Magnesite.

7. Which of the following metals is obtained by leaching its ore with dilute cyanide solution ?

(A) Silver (B) Titanium

(C) Vanadium (D) Zinc.

8. The natural materials from which an element can be extracted economically are called

(A) Ores (B) Minerals

(C) Gangue (D) None of the above.

9. Malachite is an ore of

(A) Iron (B) Zinc

(C) Copper (D) Mercury

10. Among the following statements the incorrect one is

(A) Calamine and siderite are carbonates

(B) Argentite and cuprite are oxides

(C) Zinc blende and iron pyrites are sulphides

(D) Malachite and azurite are ores of copper.

ANSWERS

1. C 2. A 3. B 4. B

5. B 6. C 7. A 8. A

9. C 10. B

Kaysonseducation s-block elements

Page 54

z

Day – 1

1. 1st group Alkali metals

Elements Atomic

Number

Electronic Configuration

Complete

gas core

With inert

Lithium (Li) 3

Sodium (Na) 11

Potassium (K) 19

Rubidium (Rb) 37

Caesium (Cs) 55

Francium (Fr) 87

1. These elements are termed as alkali metals because they all are highly reactive which form

strongly alkaline oxides and hydroxides.

2. Do not occur free in nature - because of their reactivity generally occur in combined state.

3. Alkali metals are good reducing agents - because of their low IE.

4. K & Cs are used in photo electric cells - because of their Low IE, they can eject when

exposed to light. Li – has highest IE, cannot be used in photo electric cell because does not release

when exposed to light.

1.1 Chemical Properties

1. Reactivity and electrode potential

All alkali metals are highly reactive because they have a strong tendency to lose the singly valence

to form unipositive ion inert gas configuration. It is the main reason that alkali metals act as

a good reducing agent.

Reducing character in gaseous state - Li < Na < K < Rb < Cs.

Reducing character in aqueous solution - Na < K < Rb < Cs < Li (due to higher –tive value of

)

Reason

(i) Li(s) Li(g) (sublimation energy)

(iii) enthalpy of hydration

s-block elements

Chapter

3


Page 55

The overall tendency for the charge depends upon the net effect of all the three steps.

has smallest size and is hydrated maximum therefore large amount of hydration

energy released in third step. The amount is so large (in third step) that it compensates the higher

energy needed to remove (in second step).

So net effect is

2. Reactivity with water

Here catch fire. Because of large reduction potential and Li is least reactive.

Imp.:- Not found in any other group because of presence of acidic hydrogen in compounds.

3. Reactivity towards oxygen

ion being a small ion has a strong positive field around it can stabilize only a small anion

where as being large cation stabilize a large anion.

Large have still weaker +tive field around them which cannot

prevent even peroxide ion to combine another oxygen atom to form superoxide

widely used as an oxidizing agent in Inorganic Chemistry.

Coloured & paramagnetic

Superoxide

4. Alkali metals get tarnished when exposed to air & moisture

Alkali metal acetylic

Oxide (Li2O) Peroxide

(Na2O2)

Super oxide

(K, Rb, Cs)

Oxide Peroxid

e

Superoxid

e


Page 56

Because they converted themselves into oxides, hydroxides & finally into carbonates

Because of it alkali metals stored in inert hydrocarbon solvents/petroleum ether/kerosene oil.

5. Reactivity with

Forms hydrides. When react with at 673K (1023K) Ionic hydrides .

1. Order of reactivity of alkali metal with decreases (due to lattice energy).

2. Ionic character of MH decreases, covalent character increases. Because the size of cation

increases, the anion hydride ion can polarize the more easily.

3. Hydrides act as a strong reducing agent liberate at anode.

4. Hydrides act with proton donor such as water, alcohols, gaseous ammonia & alkynes liberate

gas.

LiH:- Used as a source of for millitory purpose and for filling metrological balloons since it

has low molecular weight.

6. Reactivity with halogens

Reactivity increases due to low IE

7. Solubility in liquid Ammonia

When ordinary light falls in the solution of alkali metal in ammonia, these ammoniated electron

get excited to higher level by absorbing energy of red region. The transmitted light is blue which

imparts blue colour to the solution.

1. When concentration increases above 3M colour change Copper bronz solution acquire

metallic luster due to formation of metal ion cluster.

2. Blue solution paramagnetic presence of unpaired electrons bronze solution

diamagnetic due to formation of electron cluster.

3. The solution is good conductor of electricity due to presence of ammoniated electron & cations.

After increase in conc conductivity decrease because - bound free unpaired electrons.

4. 2n positiveness of impurities (Fe) or catalyst.

Metal Amide


Page 57

8. Oxides & hydroxides

Basic character of oxide

Increases due to low IE

1.2 Anomalous behaviour of Li

1. Very small size of atom/ion.

2. Higher polarizing power (due to high charge/size ratio) resulting in increased covalent character

of their compound responsible for their solubility in organic solvents.

3. Comparatively high I.E. & low electropositive character.

4. Non availability of d-orbital.

5. Strong intermetallic bonding.

Resemblance of Li with Mg (Diagonal relationship)

Mainly due to the similarity in sizes of their atoms (Li = 152 pm, Mg = 160 pm) & their ions (Li+

= 76 pm & Mg2+

=72 pm). (Similar changes radius ratio.)

1.3 Similarities

1. Similar electronegativity (Li = 0.98 & Mg = 1.2).

2. Both are very hard.

3. Li(OH) & weak bases.

4. Form Nitrides

5. Hydroxides & carbonates decompose on heating.

6. Can form only oxides not peroxide or superoxides.

7. Nitrates decompose on heating and give

8. Hydroxides, carbonates, oxalates, phosphates, fluoride sparingly soluble in water.

9. Do not form solid bicarbonates (due to large size of bicarbonates).


Page 58

10. Covalent character of soluble in ethanol, deliquescent & crystalline from aq.

Solution as hydrates

1.4 Imp. Points

1. Except layer structure, all other monoxides-

Anti – fluorite structure.

2 used as a source of oxygen in submarine, space shuttle & in emergency breathing

apparatuses i.e., oxygen mask.

3. LiOH is used to remove from exhaled air in confirmed quarters like submarine and space

vehicles.

4. Li cannot be store in paraffin because of its low density it will float. It is kept wrapped in

paraffin wax.

5. All Alkali metals exist as bcc with co-ordination no. 8.

6. Formation of Amalgam with Hg & Alkali metals are highly exothermic reaction.

From breathe

Documents

Chapter 1 Basic Concept of Periodic Table - Online...1.1 Periodic Table 1.2 Periodicity of Properties As per modern periodic law, physical and chemical properties of the element are